Structure and Dynamics of Iron Pentacarbonyl † § ‡ § ∥ ⊥ # Peter Portius,*, , Michael Bühl, Michael W

This is an open access article published under an ACS AuthorChoice License, which permits copying and redistribution of the article or any adaptations for non-commercial purposes. Article Cite This: Organometallics 2019, 38, 4288−4297 pubs.acs.org/Organometallics Structure and Dynamics of Iron Pentacarbonyl † § ‡ § ∥ ⊥ # Peter Portius,*, , Michael Bühl, Michael W. George, , Friedrich-Wilhelm Grevels, , § and James J. Turner*, † Department of Chemistry, The University of Sheffield, Western Bank, Sheffield S3 7HF, United Kingdom ‡ School of Chemistry, University of St. Andrews, St. Andrews, Fife KY16 9ST, United Kingdom § School of Chemistry, University of Nottingham, University Park, Nottingham NG7 2RD, United Kingdom ∥ Department of Chemical and Environmental Engineering, University of Nottingham Ningbo China, 199 Taikang East Road, Ningbo 315100, China ⊥ Max-Planck-Institut für Bioanorganische Chemie, Stiftstraße 34-36, D-45470 Mülheim an der Ruhr, Germany *S Supporting Information ABSTRACT: The dynamics of CO ligand scrambling in Fe(CO)5 has been investigated by linear infrared spectroscopy in super- critical xenon solution. The activation barrier for the Berry pseudorotation in Fe(CO)5 was determined experimentally to be ± −1 Ea = 2.5 0.4 kcal mol by quantitative analysis of the temperature-dependent spectral line shape. This compares well −1 with the range of Ea/(kcal mol ) = 2.0 to 2.3 calculated by various DFT methods and the value of 1.6 ± 0.3 previously obtained from 2D IR measurements by Harris et al. (Science 2008, 319, 1820). ··· The involvement of Fe(CO)5 Xe interactions in the ligand scrambling process was tested computationally at the BP86-D3/ AE2 level and found to be negligible. ■ INTRODUCTION It is usually assumed that the mechanism involves the Berry 6 1 pseudorotation (Figure 2). Attempts to resolve the structure Since the synthesis of Fe(CO)5 in 1891, there has been a great deal of interest in its chemistry, structure, and bonding, in particular the dynamics of the scrambling of the ligands. Fe(CO)5 has a D3h-symmetric structure in the gas phase (cf. Figure 1).2 In 1958, Cotton et al.3 observed that the 13C NMR Downloaded via UNIV OF ST ANDREWS on November 12, 2019 at 16:09:29 (UTC). Figure 2. Geometries relevant for the Berry pseudorotation model of Fe(CO) and for the DFT calculations in this paper. See https://pubs.acs.org/sharingguidelines for options on how to legitimately share published articles. 5 have been carried out in the solid state at low temperature and have resulted in some disagreement,7,8 which is, however, of little relevance to understanding the behavior in solution. That it was possible to freeze the scrambling was shown by Turner 9 Figure 1. Ball-and-stick model of the D -symmetric structure of and colleagues using a combination of polarized photolysis 3h and IR spectroscopy in a CO matrix at 20 K. Fe(CO)5. Fe, lilac; C, gray; O, red. A large number of DFT calculations on Fe(CO)5 (and other metal carbonyls) have been carried out. Most of them were concerned with structure, and particularly with the difference spectra showed only one line at all available temperatures. − − Later work4 confirmed and extended this down to −170 °C. between the axial and equatorial Fe C and C O bond lengths as well as the dissociation energy of the ligand decoordination Thus, the exchange among the CO groups must be very fast. In → rather subtle NMR experiments, Sheline and Mahnke5 reaction, Fe(CO)5 Fe(CO)4 + CO, and the vibrational estimated that at room temperature, CO scrambling occurs − at a rate of about 1.1 × 1010 s 1 with an activation energy of Received: August 16, 2019 − ∼1.13 kcal mol 1. Published: October 17, 2019 © 2019 American Chemical Society 4288 DOI: 10.1021/acs.organomet.9b00559 Organometallics 2019, 38, 4288−4297 Organometallics Article frequencies. Several authors have considered the energy ff di erence between the D3h-symmetric ground state and the top of the barrier in the Berry mechanism (C4v). Schaefer and colleagues10 calculated the barrier height using various basis sets and obtained values of 2.25 kcal mol−1 (DZ B3LYP), 2.28 kcal mol−1 (DZP BP86), and 2.33 kcal mol−1 (DZP B3LYP) with the stated methods. In an important paper, Harris and co- workers11 estimated the barrier height to be 2.13 kcal mol−1 (BP86 with the basis sets 6-31+G(d) for C and O, and LANL2DZ for Fe). More recently, Couzijn et al.12 obtained a value of 2.0 kcal mol−1 at the B3PW91/SDD(d) level of theory. The relevance of these data will be outlined shortly. We have calculated the barrier height at the BP86, PBE, PBE0, and CCSD(T) levels of theory and obtained values between 2.0 −1 ν and 2.3 kcal mol ; see the Supporting Information (SI) for Figure 3. IR spectrum in the (CO) region of Fe(CO)5 in 2- details of the calculations. Thus, the calculation of the barrier methylpentane at −140 °C. height is remarkably independent of the DFT method. However, obtaining good experimental data for the barrier and 2 are assigned to the ν(CO) vibrations that transform as ″ ′ height and the kinetics of the Berry pseudorotation is a much the a2 and e irreducible representations of D3h-symmetric 12 more challenging problem. Fe( CO)5, respectively; those labeled 3, 4, 5, 6 arise from 13 12 The study of dynamics requires experiments to be Fe( CO)( CO)4 (see the SI for a full force constant analysis) 13 14,15 conducted over a broad range of temperatures, and with very due to naturally occurring CO. The two fundamental a′ ν small barriers in particular, one needs to be able to extend this (CO) vibrations are not active in the IR under D3h symmetry to very low ones. While there is no doubt that the structure of but become active if the symmetry is reduced slightly to C2v; the bands labeled 7 and 8 are assigned to these a′ vibrations. If Fe(CO)5 in the gas phase has D3h symmetry, the complex can undergo considerable distortion in various solvents. Elegant the distortion is considerable, the degeneracy of the e′ experiments by Rose-Petruck and colleagues13 using IR vibrations is removed. spectroscopy probed the temperature dependence of the As the temperature is raised, bands 7 and 8 disappear spectrum in the region of the ν(CO) stretches. With the because the concentration of the distorted structure decreases support of DFT calculations, they were able to show that (see Figure 4). It should also be noted that bands 5 and 6 particularly in benzene and increasingly fluorinated derivatives, the structure of Fe(CO)5 distorts to C2v-orC4v-symmetric geometries. The authors also supplied thermodynamic parameters connecting the D3h structure with the various distorted structures as shown in eq 1: Fe(CO)5 + solvent → Fe(CO)5 ··· solvent ()DCC324hvv(/) (1) In pentafluorobenzene, for instance, the parameters ΔH = −3.59 ± 0.68 kcal mol−1, ΔS = −8.43 ± 1.83 cal K−1 mol−1, and ΔG = −1.08 kcal mol−1 can be used to describe the equilibrium between the two structures at room temperature. According to these data, it can be concluded that the equilibrium lies well to the right (10.6% D3h, 89.4% C2v) and ν that the (CO) IR spectrum is dominated by the distorted ν structure. However, as the temperature is raised, and assuming Figure 4. IR spectrum in the (CO) region of Fe(CO)5 in 2- methylpentane at 20 °C. ΔH remains roughly constant, the negative entropy change will cause a shift of the equilibrium to the left. If the interaction between Fe(CO)5 and cyclohexane is presumed to be weak, it appear to have coalesced at this temperaturea fact that will is not surprising that the experimental evidence for a complex be discussed at a later stage. However, caution must be is weak, and the authors concluded that at room temperature, exercised in using even saturated hydrocarbons as supposedly “ ” 13 Fe(CO)5 is nearly undisturbed D3h in cyclohexane. With inert solvents. What solvents could be used? Figure 5 shows the negative entropy changes being involved, there will be an ff the spectra of Fe(CO)5 in liquid krypton and at two di erent even lesser distortion of the structure at higher temperatures. concentrations in liquid xenon. However, since this paper is concerned with the dynamic It is clear that even at this low temperature there is no behavior of Fe(CO)5, more information is needed about both evidence for bands 7 and 8. Under the assumption that ΔS is structures and spectra in a variety of solvents. The following ··· negative (see later), the concentrations of Fe(CO)5 Kr and describes new experimental and computational evidence for Fe(CO) ···Xe will be zero at room temperature and above. It fl 5 the barrier in this prototypical uxional molecule. will be shown later that an accurate force field is required for the investigation of the dynamics of Fe(CO) . The assignment ■ RESULTS AND DISCUSSION 5 of the energy-factored force constants of Fe(CO)5 is Figure 3 shows the ν(CO) region of the IR spectrum of straightforward and follows that of Bor.15 The details of the − ° Fe(CO)5 in 2-methylpentane at 140 C. The bands labeled 1 calculation are given in the SI. Since the experiments described 4289 DOI: 10.1021/acs.organomet.9b00559 Organometallics 2019, 38, 4288−4297 Organometallics Article fi ··· Figure 6. Energy pro le for Fe(CO)5 Xe as a function of the ··· Fe(CO)5 Xe distance (all other parameters optimized) calculated at the BP86/AE2 (○) (a purely repulsive potential) and BP86-D3/AE2 (●) levels.

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